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Number of moles is inversely proportional to molar mass.
Percentage yield = (0.45 ÷ 0.75) × 100 = 60%.
The balanced equation is 3Fe + 4H₂O → Fe₃O₄ + 4H₂. Their sum is 12.
Avogadro's law relates gas volume directly with the number of molecules at constant temperature and pressure.
The sample contains 0.25 mole of CO₂. Since one mole weighs 44 g, the mass is 11 g.
Half a mole of CO₂ occupies 11.2 dm³ at STP.
The molar mass divided by Avogadro's number gives the mass of one molecule.
Sixty-four grams of SO₂ equal one mole, producing one mole of SO₃.
One atomic mass unit is defined as one-twelfth the mass of a carbon-12 atom.
Actual yield equals 80% of theoretical yield. Therefore, 0.80 × 5 = 4 moles.
This represents 0.5 mole of water. Half of 18 g equals 9 g.
The balanced equation directly provides the ratio.
One mole always contains 6.022 × 10²³ elementary particles.
One mole of nitrogen produces two moles of nitrogen dioxide. Therefore, 0.5 mole yields one mole.
One mole occupies 22.4 dm³ at STP, so two moles occupy 44.8 dm³.
Forty-eight grams of magnesium equal two moles, producing two moles of MgO. The mass becomes 80 g.
Each NH₃ molecule contains three hydrogen atoms; therefore one mole of NH₃ contains three moles of hydrogen atoms.
Half a mole contains half of Avogadro's number of molecules.
Glucose contains six carbon atoms per molecule. Therefore, 0.5 mole of carbon atoms corresponds to 0.5 ÷ 6 = 0.083 mole of glucose.
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